The activation energy of a reaction can be lowered by:

using a positive catalyst

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increasing temperature

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decreasing temperature

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increasing concentration of the reactants

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Solution

The correct option is A using a positive catalyst
With the use of a catalyst, the transition state of the reaction lower down and hence the activation energy of the reaction decreases.

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Similar questions

Q. Assertion: Increasing the concentration of reactants will cause a reaction to proceed faster.
Reason: More reactants lowers the activation energy of a reaction.

The energy of activation for a reaction at $300 K$ is $100 k J m o l^{- 1}$ . For same concentration, presence of a catalyst lowers the energy of activation by $75 %$ . Calculate the value of
${log}_{10} (\frac{r_{2}}{r_{1}})$
$r_{2} = rate in presence of catalyst$
$r_{1} = rate in absence of catalyst$

Q. A catalyst lower the energy of activation by

25 %

. The temperature at which rate of uncatalysed reaction would be equal to that of the catalyzed one at

27^{o} C

is:

Q. Assertion :If the activation energy of a reaction is zero, temperature will have no effect on the rate constant. Reason: Lower the activation energy, faster is the reaction.

Activation energy is always lowered by positive catalyst.

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The activation energy of a reaction can be lowered by:

The correct option is A using a positive catalystWith the use of a catalyst, the transition state of the reaction lower down and hence the activation energy of the reaction decreases.

The correct option is A using a positive catalyst
With the use of a catalyst, the transition state of the reaction lower down and hence the activation energy of the reaction decreases.